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CHEM 106 > Exam 2 > Flashcards

Exam 2 Flashcards

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1
Q

What are the rules for manipulating the equilibrium constant?

A
  1. Reverse rxn = 1/k
  2. multiply rxn coefficients = K raised to multiplier
  3. Add two rxns = multiply k’s
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2
Q

What affects equilibrium/K?

A

Temperature

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3
Q

What does not affect equilibrium/K?

A
  1. Presence of catalysts
  2. Adding non-agents
  3. Solids and pure liquids
  4. Changing P/V
  5. Differing initial concentrations
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4
Q

How does change in T affect exothermic and endothermic rxns differently?

A

Endothermic- K gets larger (right shift) when T increases and vise versa
Exothermic- K gets smaller (left shift) when T increases

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5
Q

How do you find delta G not of a rxn?

A

Products minus reactants (multiplied by stoicheometric coefficient)

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6
Q

How do you derive delta G equations from equation sheet?

A

See equation sheet

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7
Q

How do you write a losing of 4 neutrons?

A

4 as coefficient, not as numerator

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8
Q

Binding energy remember

A

Do not forget to account for electrons (if applicable)
nucleons - nucleus
Atomic mass - need to subtract electrons
Nucleic mass- no subtraction necessary

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9
Q

Meaning of A = kN

A 
A = activity (disintigrations/s)
k = k value calculated from half-life equation
N = number of nuclei present, found from atomic mass and Avogadro's number
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10
Q

pKa equation

A

pX = -logX

pKa = -logKa
Ka = 10^-pKa
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11
Q

Meaning of Sv and Gy

A 
Sv = Sievert = effective exposure. Found by multiplying Gy by RBE for that specific type of radiation
Gy = Joules/Kg tissue mass
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12
Q

Acid strength trends

A

Binary acids - increase going down the row
Oxoacids - increase going up the row (except F)
Within oxoacid series - the more O present, the stronger the acid
The stronger the acid, the weaker the conjugate base

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13
Q

Factors affecting acid strength

A

Polarity- the more polar, the stronger the acid
Electronegativity- the more electronegative, the stronger the acid
Stability of conjugate base- the more stable the conjugate base, the stronger the acid
Strength of conjugate base- the weaker the conjugate base, the stronger the acid

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14
Q

Factors affecting base strength

A

Electron donating group present- strengthens base
Electron withdrawing group present - weakens base
The stronger the base, the weaker the conjugate acid

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15
Q

pH equations

A

pH = -log[H+}
[H+] = 10 ^-pH
pH +pOH = 14
[H+][OH-] = 1x10E-14

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16
Q

pOH equations

A 
pOH = -log[OH-]
[OH-] = 10^-pOH
17
Q

Classify weak or strong: HI

A

strong

18
Q

Classify weak or strong: HBr

A

strong

19
Q

Classify weak or strong: HCl

A

strong

20
Q

Classify weak or strong: HClO3

A

strong

21
Q

Classify weak or strong: HClO4

A

strong

22
Q

Classify weak or strong: HNO3

A

strong

23
Q

Classify weak or strong: H2SO4

A

strong

24
Q

Classify weak or strong: HF

A

weak

25
Q

Classify weak or strong: CH3COOH

A

weak

26
Q

H3PO4

A

weak

27
Q

Review how to calculate pH of acid or base solution

A

Use Ka and rice table. Find equilibrium concentrations, if none are provided see if you can use small k assumption (Ka &laquo_space;1). If not, use the quadratic formula to solve for equilibrium concentrations. Take -log of [H+] to find pH.

28
Q

What is the relationship between Ka and acid/base strength?

A

The larger the Ka value, the stronger the acid/base

29
Q

Definition of Arrhenius acids and bases

A

Arrhenius acids donate H+ ions and is specific to reactions happening in water.
Arrhenius bases accept H+ ions and are also specific to reactions happening in water

30
Q

Meaning of Kw

A

Special equilibrium constant for water.
Ka x Kb = 1E-14
[H+][OH-}= 1E-14

31
Q

If a solution has a pH of 7 is it acidic, basic, or neutral?

A

Neutral

32
Q

If a solution has a pH of 3 is it acidic, basic or neutral?

A

Acidic

33
Q

If a solution has a pH of 13, is it acidic, basic or neutral?

A

Basic

34
Q

If a solution has a pOH of 3, is it acidic, basic or neutral?

A

Basic

35
Q

How many more times acidic is a pH 3 solution compared to a pH 6 solution?

A

1,000x

CHEM 106 (1 decks)

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